Module 2: Foundations in Chemistry; Electrons and Bonding

?
  • Created by: jstellen
  • Created on: 20-10-16 17:07

Electronic Structure

  • Shells are made up of orbitals; orbitals can hold up to 2 electrons
  • Each shell can hold 2n squared electrons
  • The number of orbitals increases with each new type of orbitals: s,1  p,3  d,5  f,7
  • two electrons fit into each orbital so the number of electrons also increases in each sub-shell:
  • s, 1x2=2  p, 2x3=6  d, 2x5=10  f, 2x7=14
  • 3d has a higher energy level then 4s
  • With the box model fill in each box with on arrow first the repeat with alternate arrows
1 of 3

Ionic Bonding and Structure

  • An ionic bond is an attraction between two oppositely charged ions
  • Ionic bonding is when one atom donates electrons to become a positive cation and the other atom recieves electrons to become a neagtive anion
  • Ionic compounds are structured in giant ionic lattices
  • Almost all ionic compounds are solids at room temp
  • Have high MP and BP due to the strong electrostatic forces of attraction between the ions
  • The larger the charges on the ions, the stronger the attraction, the higher the BP
  • The larger the size of the ion, the stronger the attraction
  • Ionic compounds dissolve in polar substances such as water. However with large charges, the attraction may be too strong for water to break down decreasing the solubility
  • Won't conduct as solids as ions are in fixed positions so there are no mobile charge carriers
  • Will conduct when molten or dissolved in water as ions are free to move so there are mobile charge carriers
2 of 3

Covalent Bonding

  • Covalent bonding is the electrostatic attraction between a shared pair of electrons and the nuclie of the bonded atoms
  • Found in: diatomic molecules, non-metallic compounds, polyatomic compounds
  • A covelent bond is the overlap of two atomic orbitals
  • The attraction is localised
3 of 3

Comments

No comments have yet been made

Similar Chemistry resources:

See all Chemistry resources »See all Electrons and Bonding resources »